. The decomposition of N₂O5 in carbon tetrachloride has been studied:2 N₂O5 (g) → 2 N₂O4 (g) + O₂(g)The concentration of N₂O5 is monitored for 1200 seconds andmeasured every 400 seconds. The data are tabulated below:[N₂O5](M)0.01.40400.01.10800.00.871200.00.68(a) Fill the blanks in the table. Note that the last column is theaverage rate of reaction.(b) Briefly explain why the rates are decreasing.time(s)At(s)Rate =-A[N₂O5]/At(M/s)A[N₂O5](M)

∆t(s) = Final time(s) - Initial time(s) ∆[N2O5] = Final [N2O5] - Initial [N2O5]

The decomposition of N₂O5 in carbon tetrachloride has been studied: 2 N₂Os (g) ->>> 2 N₂O4 (g) + O₂(g) The concentration of N₂O5 is monitored for 1200 seconds and measured every 400 seconds. The data are tabulated below: time(s) [N₂O5] (M) 1.40 At(s) A[N₂O5](M) - Rate =L A[N₂O5]/At(M/s) - 0.0 400.0 1.10 800.0 0.87 1200.0 0.68 (a) Fill the blanks in the table. Note that the last column is the average rate of reaction. (b) Briefly explain why the rates are decreasing. --

The decomposition of N₂O5 in carbon tetrachloride has been studied: 2 N₂Os (g) ->>> 2 N₂O4 (g) + O₂(g) The concentration of N₂O5 is monitored for 1200 seconds and measured every 400 seconds. The data are tabulated below: time(s) [N₂O5] (M) 1.40 At(s) A[N₂O5](M) - Rate =L A[N₂O5]/At(M/s) - 0.0 400.0 1.10 800.0 0.87 1200.0 0.68 (a) Fill the blanks in the table. Note that the last column is the average rate of reaction. (b) Briefly explain why the rates are decreasing. --

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased
Write the net reaction for the following elementary processes Step 1: NO(g) + NO(g) = N2O2(g) (slow) Step 2: N2O2(g) + O2(g) = NO2(g) + NO2(g) How would I go about solving this question?
Nitrogen monoxide reacts with oxygen to give nitrogen dioxide. 2NO(9) + 02 (9) → 2NO: (9) The rate law is A[NO] At - k[NO]°[02] where the rate constant is 1.16 x 10-5 L/(mol? . s) at 339°C. A vessel contains NO and Oz at 339°C. The initial partial pressures of NO and Oz are 157 mmHg and 348 mmHg, respectively. What is the rate of decrease of partial pressure of NO? (Hint: From the ideal gas law, obtain an expression for the molar concentration of a particular gas in terms of its partial pressure.) Rate =
The oxidation of ammonia produces nitrogen and water via the following reaction: 4NH3(g) + 302(g) → 2N2(g) + 6H₂O(A) Suppose the rate of formation of H₂O(A) is 3.0 mol/(Ls). Which of the following statements is true? The rate of consumption of NH3 is 2.0 mol/(L. s). The rate of consumption of O₂ is 2.0 mol/(L. s). The rate of formation of N₂ is 1.3 mol/(Ls). The rate of formation of N₂ is 2.0 mol/(Ls). The rate of consumption of NH3 is 0.50 mol/(L. s).
Q3
onsider the reaction of ozone (0.) with nitrogen monoxide (NO), hich occurs in smog. What effect would each of the following changes ave on the rate of this reaction? O3(g) + NO(g) O2(g) + NO2(g) nereasing the concentration of O, ecreasing the concentration of NO ncreasing the temperature ecreasing the temperature
1. At elevated temperatures, nitrous oxide decomposes according to the equation2N2O(g)⟶2N2(g)+O2(g) Time (min) 0 60 90 300 600 [N2O] 0.250 0.228 0.216 0.128 0.0630 Given the following data, determine whether the reaction is zeroth, first, or second order. a) first b) second c) zeroth
The oxidation of ammonia produces nitrogen and water via the reaction: 4NH3(g) + 302(g) ---> 2N2(g) + 6H₂O(g). If the rate of formation of nitrogen gas is 2.0 mol/(Los), then the rate at which: water is formed is also 2.0 mol/(Los) oxygen reacts is 1.5 mol/(Los) ammonia reacts is 0.5 mol/(L •s) ammonia reacts is 4.0 mol/(Los) water is being formed is 0.67 mol/(Los)
Given the following data for the reaction AB, determine the frequency factor, A, of the reaction to three significant figures. k(5¹) 0.730 0.739 T(K) 2.50 102 4.50 x 10² a) -0.287 s1¹ b) 2.05 ¹ Od 0.719 s¹¹ d) 0.287 s e) 0.750 1
Consider the reaction: 2NO(g) + O2(g) → 2NO2(g) Suppose that a particular moment during the reaction nitric oxide (NO) is reacting at a rate of 0.022 M/s. At what rate is molecular oxygen reacting? M Molecular oxygen is (select) at a rate of